Ch.2 - Atoms, Molecules, and Ions

Problem 55

Chapter 2, Problem 55

Fill in the gaps in the following table: Symbol 59Co3+ Protons 34 76 80 Neutrons 46 116 120 Electrons 36 78 Net charge 2+

Verified step by step guidance

Identify the number of protons for each element using the atomic number, which is equal to the number of protons.

Calculate the number of electrons for each ion by considering the net charge: Electrons = Protons - Charge.

Determine the number of neutrons by subtracting the number of protons from the mass number: Neutrons = Mass Number - Protons.

For the given symbol 59Co3+, identify the number of protons from the periodic table (Co has 27 protons) and calculate the number of electrons considering the charge (27 - 3 = 24 electrons).

Fill in the missing values in the table using the calculated numbers of protons, neutrons, and electrons for each element or ion.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Atomic Structure

Atomic structure refers to the composition of an atom, which includes protons, neutrons, and electrons. Protons are positively charged particles found in the nucleus, while neutrons are neutral particles also located in the nucleus. Electrons are negatively charged and orbit the nucleus. The number of protons determines the element, while the balance of protons and electrons defines the atom's charge.

Ions and Charge

Ions are atoms or molecules that have gained or lost one or more electrons, resulting in a net electric charge. A cation, like Co3+, has lost electrons, leading to a positive charge. The net charge of an ion is calculated by subtracting the number of electrons from the number of protons. Understanding how to determine the charge is essential for filling in the gaps in the provided table.

Isotopes

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. This difference in neutrons results in varying atomic masses. For example, cobalt (Co) can have isotopes with different neutron counts, affecting its stability and nuclear properties. Recognizing isotopes is crucial for accurately completing the table regarding neutrons and atomic mass.

Recommended video:

Guided course

04:36

Isotopes

Related Practice

Textbook Question

How many of the indicated atoms are represented by each chemical formula: (b) oxygen atoms in Ca(ClO₃)₂ (c) hydrogen atoms in (NH₄)₂HPO₄?

Textbook Question

Write the molecular and structural formulas for the compounds represented by the following molecular models:

Textbook Question

Write the molecular and structural formulas for the compounds represented by the following models:

Textbook Question

Fill in the gaps in the following table:

Symbol 31P3-

Protons 34 50

Neutrons 45 69 118

Electrons 46 76

Net charge 2- 3+

Textbook Question

Each of the following elements is capable of forming an ion in chemical reactions. By referring to the periodic table, predict the charge of the most stable ion of each: c. K

Textbook Question

Using the periodic table, predict the charge of the most stable ion of the following elements: d. Br